Consider the reaction equilibrium 2SO2(g)+O2(g)2 SO3 (g); ΔHº = -198 kJOn the basis of Le Chatelier's principle, the condition favourable for the forward reaction is -[AIEEE-2003]a)Lowering the temperature and increasing the pressureb)Any value of temperature and pressurec)Lowering of temperature as well as pressured)Increasing temperature as well as pressureCorrect answer is option 'A'. Can you explain this answer?

Question

Consider the reaction equilibrium 2SO2(g)+O2(g)2 SO3 (g); &Delta;H&ordm; = -198 kJOn the basis of Le Chatelier's principle, the condition favourable for the forward reaction is -[AIEEE-2003]a)Lowering the temperature and increasing the pressureb)Any value of temperature and pressurec)Lowering of temperature as well as pressured)Increasing temperature as well as pressureCorrect answer is option 'A'. Can you explain this answer?

Answer

The correct answer is option A

ACCORDING TO LE CHATELIER'S PRINCIPLE

TEMPERATURE
if we increase temperature equilibrium will shift that direction which proceeds an endothermic reaction but the reaction given in question is exothermic so we have to decrease temperature to proceed forward.

PRESSURE
at equilibrium if we increase pressure equilibrium will shift that direction which has less number of moles but in given reaction products have less no. of moles than reactant that's why we increase pressure.

Answer

ACCORDING TO LE CHATELIER'S PRINCIPLE

TEMPERATURE
if we increase temperature equilibrium will shift that direction which procedes endothermic reaction but the reaction given in question is exothermic so we have to decrease temperature to proceed reaction forward.

PRESSURE
at equilibrium if we increase pressure equilibrium will shift that direction which have less number of moles but in given reaction product have less no. of moles than reactant that's why we increase pressure.

Answer

The reaction equilibrium you provided is missing the reactant and product coefficients. The balanced equation for the reaction is:

2SO2(g) + O2(g) ⇌ 2SO3(g)

In this reaction, sulfur dioxide (SO2) and oxygen (O2) react to form sulfur trioxide (SO3). The reaction can proceed in both directions, with SO2 and O2 forming SO3, and SO3 decomposing back into SO2 and O2.

When the reaction reaches equilibrium, the concentrations of the reactants and products remain constant over time. The equilibrium constant (K) for this reaction is defined as the ratio of the product concentrations to the reactant concentrations, with each concentration raised to the power of its coefficient in the balanced equation.

K = [SO3]^2 / ([SO2]^2 * [O2])

The value of the equilibrium constant depends on temperature, and it indicates the relative concentrations of the reactants and products at equilibrium. A larger value of K means that the products are favored at equilibrium, while a smaller value of K means that the reactants are favored.

To calculate the value of K, you would need to know the concentrations of the reactants and products at equilibrium.

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